Question

In: Chemistry

2 ml MTF-HCL of A (50 mg/ml, Phosphate buffer, ph 4.2) 1) What does this sentence...

2 ml MTF-HCL of A (50 mg/ml, Phosphate buffer, ph 4.2)

1) What does this sentence mean?

2) What is the weight percent of MTF-HCL

Metformin hydrochloride is a drug and we must dissolve this drug in a phosphate buffer .

I do not get the phrase in the article which is stated above. How much of this drug is dissolving in this buffer to obtain 2 mL of final solution.

Solutions

Expert Solution



Related Solutions

You must make a sodium phosphate buffer (500 ml at 50 mM) at a pH value...
You must make a sodium phosphate buffer (500 ml at 50 mM) at a pH value of 6.8. Assume that the pKa is 7.0. MW oh NaH2PO4 = 138g/mol. MW of NaH2PO4 = 268 g/mol Show the weak acid base reaction with proper structures. use the Henderson/ Hasselbalch relationship to obtain molarity of each species. Calculate the grams of each salt required.
Buffer 1) 100 mL of 0.50 M sodium phosphate buffer, pH 7.0 MW; 137.99
Buffer 1) 100 mL of 0.50 M sodium phosphate buffer, pH 7.0 MW; 137.99
1. Using a 0.20 M phosphate buffer with a pH of 6.9, you add 0.80 mL...
1. Using a 0.20 M phosphate buffer with a pH of 6.9, you add 0.80 mL of 0.46 M HCl to 53 mL of the buffer. What is the new pH of the solution? (Enter your answer to three significant figures.) 2. Using a 0.20 M phosphate buffer with a pH of 6.9, you add 0.80 mL of 0.46 M NaOH to 53 mL of the buffer. What is the new pH of the solution? (Enter your answer to three...
find the pH of a 40 mL buffer solution + 1.0 mL of 6.0 M HCl...
find the pH of a 40 mL buffer solution + 1.0 mL of 6.0 M HCl (aq) I know this question is pretty simple, but do I need to know what the buffer is made of? Is it important? if not how would I set up the ICE table? thank you!
You are instructed to create 300. mL of a 0.34 M phosphate buffer with a pH...
You are instructed to create 300. mL of a 0.34 M phosphate buffer with a pH of 7.3. NaH2PO4 is the acid component of the buffer. Na2HPO4 is the base component of your buffer. What is the molarity needed for the acid component of the buffer? What is the molarity needed for the base component of the buffer? How many moles of acid are needed for the buffer? How many moles of base are needed for the buffer? How many...
How would you make up 100 ml of 50 mM Tris-HCl buffer at pH 7.4, using...
How would you make up 100 ml of 50 mM Tris-HCl buffer at pH 7.4, using the 0.5 M Tris base stock solution, and any other required materials?
2.0 mL of 0.5M HCl was added to 50 mL of 0.5M Formate-formic acid buffer at...
2.0 mL of 0.5M HCl was added to 50 mL of 0.5M Formate-formic acid buffer at pH 3.6. (pKa= 3.75) What is the resulting pH after the addition of HCl? 2.0 mL of 0.5M HCl was added to 50 mL of 0.0625M Formate-formic acid buffer at pH 3.6. (pKa= 3.75) What is the resulting pH after the addition of HCl? 1.0 mL of 0.6M NaOH was added to 10 mL of 0.5M Acetate-acetic acid buffer at pH 4.2. What is...
Using a 0.25 M phosphate buffer with a pH of 6.7, you add 0.72 mL of...
Using a 0.25 M phosphate buffer with a pH of 6.7, you add 0.72 mL of 0.45 M HCl to 49 mL of the buffer. What is the new pH of the solution? (Enter your answer to three significant figures.)
Using a 0.20 M phosphate buffer with a pH of 6.8, you add 0.72 mL of...
Using a 0.20 M phosphate buffer with a pH of 6.8, you add 0.72 mL of 0.50 M HCl to 53 mL of the buffer. What is the new pH of the solution? (Enter your answer to three significant figures.)
Using a 0.25 M phosphate buffer with a pH of 6.0, you add 0.79 mL of...
Using a 0.25 M phosphate buffer with a pH of 6.0, you add 0.79 mL of 0.45 M NaOH to 59 mL of the buffer. What is the new pH of the solution? (Enter your answer to three significant figures.)
ADVERTISEMENT
ADVERTISEMENT
ADVERTISEMENT